Question

A student is given 1.6604 g of an unknown copper compound. Following the isolation by displacement...

A student is given 1.6604 g of an unknown copper compound. Following the isolation by displacement by Mg, 0.7193 g of Cu metal is recovered.

a.What is the percentage of Cu in the sample?

b.What is the formula weight of the compound? (Assume one mole of the compound contains one mole of copper.)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

mass of compound = 1.6604 grams

mass of copper = 0.7193 grams

% of copper= mass of copper/mass of compound x100

% of copper = 0.7193/1.6604 x100 = 43.3%

% of copper = 43.3%

b) mass of copper = 0.7193 grams

molar mass of compound = 63.5 gram/mole

number of moles of copper = 0.7193/63.5 = 0.0113 moles

number of moles = mass/molar mass of compound

molar mass of compound = mass/number of moles = 1.6604/0.0113 = 146.9 gram/mole

formula weight of the compound = 146.9 gram/mole.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A solution contains 11.45 g of unknown compound dissolved in 50.0 mL of water. (Assume a...
A solution contains 11.45 g of unknown compound dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -4.73 ∘C. The mass percent composition of the compound is 53.31% C, 11.19% H, and the rest is O. What is the molecular formula of the compound? Express your answer as a molecular formula.
A 0.4958 g sample of a pure soluble chloride compound is dissolved in water, and all...
A 0.4958 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 1.0569 g. What is the mass percentage of chlorine in the original compound? % A student determines the copper(II) content of a solution by first precipitating it as copper(II) hydroxide, and then decomposing the hydroxide to copper(II)...
In a freezing point-depression experiment where an unknown molecular compound is added to cyclohexane, a student...
In a freezing point-depression experiment where an unknown molecular compound is added to cyclohexane, a student collects the following data. Mass of cyclohexane: 3.497772 g Mass of unknown sample: 0.031104 g Molality of unknown sample: 0.07157 mol/kg Compute the molar mass in g/mol of the unknown sample from the studen'ts data. watch significant figures
An unknown compound has the following chemical formula: Ca(OH)x where x stands for a whole number....
An unknown compound has the following chemical formula: Ca(OH)x where x stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 6.9 mol of oxygen and 3.5 mol of calcium. Write the complete chemical formula for the unknown compound.
41) Combustion analysis of a 0.675 g sample of an unknown compound that contains only carbon,...
41) Combustion analysis of a 0.675 g sample of an unknown compound that contains only carbon, hydrogen, and oxygen gives 0.627 g of CO2 and 1.534 g of H2O. The molecular mass of the unknown is Select one: A. C6H12O2. B. C3H6O. C. C9H18O3. D. unable to be determined from this data. 42) How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l) Select...
One way in which the useful metal copper is produced is by dissolving the mineral azurite,...
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from...
1.A 0.5538 g sample of a pure soluble bromide compound is dissolved in water, and all...
1.A 0.5538 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide ion is precipitated as AgBr by the addition of an excess of silver nitrate. The mass of the resulting AgBr is found to be 1.1298 g. What is the mass percentage of bromine in the original compound? % 2. A student determines the manganese(II) content of a solution by first precipitating it as manganese(II) hydroxide, and then decomposing the hydroxide to...
An empirical formula is the lowest whole number ratio of the elements in a compound and...
An empirical formula is the lowest whole number ratio of the elements in a compound and provides information about the composition of a compound. For instance, the compound sodium sulfate decahydrate has the chemical formula Na2SO4•10H2O. This formula conveys the information that there are ten water molecules per two sodium ions per one sulfate ion. You might wonder: “How were these ratios determined?” To answer the question it is necessary to recognize that the ratio of atoms (or ions) is...
In the lab, you grind up 2.205 g of an unknown compound and dissolve it in...
In the lab, you grind up 2.205 g of an unknown compound and dissolve it in 250 mL of water. You take 5 mL of this solution and dilute it to a volume of 125 mL. Using a titration, you measure the concentration of the resulting solution to be 1.96*10-3 M. Determine which of the following could be the formula of the compound. Show your work. You will need to work backwards and remember that the molar mass is equal...
1) Which of the following is NOT valid reasoning for these results: A student begins with...
1) Which of the following is NOT valid reasoning for these results: A student begins with 5.00 g of an unknown mixture and recovers 2.91 g of copper sulfate and 2.58 g of salicylic acid? (Check all that apply.) One or more of the fractions was not fully dried The mass of the filter paper was not subtracted from the mass of the crystals The reaction spontaneously created more mass 2) What is the percent recovery of the sample if...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT